Write balanced chemical equations that correspond to the following equilibrium constant expressions. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) a. K = b. K = C. K = [H₂O₂)² [H₂O]² [0₂] + [Ag+]²[S0₁²] + [HSO,¯] [H₂O+] [H₂SO3] + T↓ TL 11 + +

For the reaction below, Kc = 1.10 x 10-8. Note Kc is sometimes called K. What is the equilibrium concentration of OH¯ if the reaction begins with 0.140 M HONH,? HONH2 (aq) + H,0 (I) = HONH3* (aq) + ОН (аq)

Calculate the number of moles of vitamin C in the tablet based on the stoichimetry from the equation given in the back ground 1000 mg is in each tablet

a) Balance the following equation and write it below: Fe (s) + Mg3(PO,), (aq) → Fe;(P 0,), (aq) + Mg(s) b) If you added 134.2 grams of Iron to an excess of Mg,(PO,)2, how many moles of Iron have you added? c) Assuming the reaction is reversible, in which direction would the equilibrium shift if Fe was removed from the solution (left, right, or no change?) d) What type of reaction is this?

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB⇌cC+dD where a, b, c, & d are the stoichiometric coefficients, the equilibrium constant is Kc=[C]c[D]d[A]a[B]b & where [A][A], [B][B], [C][C], and [D][D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead of the equilibrium constant, Kc.Qc=[C]tc[D]td[A]ta[B]tb where each concentration is measured at some arbitrary time t. Part A  A mixture initially contains AA, BB, and CC in the following concentrations: [A]= 0.700 M, [B]= 1.40 M, & [C]= 0.550 M. The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A]= 0.520 M & [C]= 0.730 M. Calculate the value of the equilibrium constant, Kc.

6. Give the equilibrium constant for the following reaction. 2PB1, (g) + 3Cl,(s) 2PCI;(g) + 3Br,(g)

A student determines that an aqueous solution that contains 0.474 M potassium hypochlorite and 0.180 M hypochlorous acid, also has an H30* concentration of 1.89x10-8 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HCIO(aq) + H2O =H30*(aq) + ClO(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K

Write the equilibrium constant expression for this reaction: 2 H* (aq) + C₂0 (aq) H₂C₂O4(aq) X S